When $22.4 \ L$ of $H_{2(g)}$ is mixed with $11.2 \ L$ of $Cl_{2(g)}$,each at $S.T.P.$,the moles of $HCl_{(g)}$ formed is equal to

$CaCO_{3(s)} + 2 HCl_{(aq)} \rightarrow CaCl_{2(aq)} + CO_{2(g)} + H_2O_{(l)}$
Consider the above reaction,what mass of $CaCl_2$ will be formed if $250 \ mL$ of $0.76 \ M \ HCl$ reacts with $1000 \ g$ of $CaCO_3$ (in $g$)?
(Given: Molar mass of $Ca, C, O, H$ and $Cl$ are $40, 12, 16, 1$ and $35.5 \ g \ mol^{-1}$,respectively)

When $12 \ L$ of $H_2$ and $11.2 \ L$ of $Cl_2$ are mixed and allowed to react according to the equation $H_{2(g)} + Cl_{2(g)} \rightarrow 2HCl_{(g)}$,what is the final composition of the mixture?

What is the approximate mass of the precipitate formed when $50 \text{ mL}$ of $16.9\%$ solution of $AgNO_3$ is mixed with $50 \text{ mL}$ of $7.45\%$ $KCl$ solution (in $\text{ g}$)? (Molar mass of $AgNO_3 = 169 \text{ g/mol}$, $KCl = 74.5 \text{ g/mol}$, $AgCl = 143.3 \text{ g/mol}$)

One mole of calcium phosphide on reaction with excess water gives

What is the maximum amount of $Cl_2$ gas produced when $1 \, g$ of $HCl$ and $1 \, g$ of $MnO_2$ are heated together (in $, g$)?